A) high hydration energy of \[L{{i}^{+}}\] ion
B) high ionization energy of \[L{{i}^{+}}\] ion
C) small size of \[L{{i}^{+}}\] ion
D) non-metallic character of \[L{{i}^{+}}\] ion
Correct Answer: A
Solution :
In alkali metals, the extent of hydration depends upon the size of ion. Smaller the size of the ion, more highly it is hydrated and greater is its hydration enthalpy. Ionic radius:\[L{{i}^{+}}<N{{a}^{+}}<{{K}^{+}}<R{{b}^{+}}<C{{s}^{+}}\] Hydrated ionic radius: \[L{{i}^{+}}>N{{a}^{+}}>{{K}^{+}}>R{{b}^{+}}>C{{s}^{+}}\] As \[L{{i}^{+}}\] ion has smaller size among all the alkali metal ions, hence greater is its hydrated ionic radius and less is its ionic mobility or conductance in its aqueous solution.
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